{"id":2794,"date":"2016-08-24T18:30:47","date_gmt":"2016-08-24T18:30:47","guid":{"rendered":"https:\/\/courses.lumenlearning.com\/umes-cheminter\/?post_type=chapter&#038;p=2794"},"modified":"2017-08-28T22:53:58","modified_gmt":"2017-08-28T22:53:58","slug":"ionic-bonding","status":"publish","type":"chapter","link":"https:\/\/courses.lumenlearning.com\/umes-cheminter\/chapter\/ionic-bonding\/","title":{"raw":"Ionic Bonding","rendered":"Ionic Bonding"},"content":{"raw":"<h1 id=\"x-ck12-SW9uaWMgYW5kIE1ldGFsbGljIEJvbmRpbmc.-chapter\">Ionic and Metallic Bonding<\/h1>\r\n<div class=\"x-ck12-data\"><\/div>\r\n<h1 id=\"x-ck12-RWxlY3Ryb24gRG90IERpYWdyYW1z\">Ionic Bonding<\/h1>\r\n<div class=\"x-ck12-data-objectives\">\r\n<ul id=\"x-ck12-Y2Q1MjBiMGQ3YjQxMjUxNWNmODU0N2IxZjliZGU3N2U.-il7\">\r\n \t<li>Define ionic compound.<\/li>\r\n \t<li>Define ionic bond.<\/li>\r\n \t<li>Use electron dot diagrams to illustrate electron transfer and ionic bond formation.<\/li>\r\n<\/ul>\r\n<\/div>\r\n<p id=\"x-ck12-ZmQ0Y2JmYmY3YzI2ODA0ODhhYTFlYTdjMTI0ZGIzZTk.-vbk\"><span class=\"x-ck12-img-inline\"><img src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images-archive-read-only\/wp-content\/uploads\/sites\/53\/2014\/08\/19211355\/20140811155231639993.jpeg\" alt=\"The sea contains a lot of salt, an ionic compound\" width=\"400\" \/><\/span><\/p>\r\n<p id=\"x-ck12-YTc2OWI2OTFjNmIwMWFlOTM5MTZhYWJkNTRjYzMzMDc.-rsp\"><strong>Does the sea really have salt in it?<\/strong><\/p>\r\n<p id=\"x-ck12-MDRhZDIxNWFjMTRjOGQ2YjBmYjMzOGExNmUzZTQ0NTE.-c1w\">We can get common table salt from several sources.\u00a0 It can be mined in the solid form in salt mines or found as a solid in deposits.\u00a0 We can also get salt from the ocean, but it really does not exist as salt when in solution.\u00a0 The sodium ions and chloride ions are dissolved, but not combined into a structure until all the water is removed.<\/p>\r\n<p id=\"x-ck12-OGExYWVjNDUzMTk5ODEyZTdkMzBlYzJmMDkzYmNjYmU.-icq\">Most of the rocks and minerals that make up the Earth\u2019s crust are composed of positive and negative ions held together by ionic bonding.\u00a0 An ionic compound is an electrically neutral compound consisting of positive and negative ions.\u00a0 You are very familiar with some ionic compounds such as sodium chloride (NaCl).\u00a0 A sodium chloride crystal consists of equal numbers of positive sodium ions (Na <sup>+ <\/sup>) and negative chloride ions (Cl <sup>\u2212 <\/sup>).\u00a0 <em>\u00a0<\/em><\/p>\r\n\r\n<h3>Ionic Bonds<\/h3>\r\n<p id=\"x-ck12-MWMxM2E0NmY3MmZkNzQ1YjdmY2Y0Y2IyODU5OTBkNmI.-ez1\">Oppositely charged particles attract each other.\u00a0 This attractive force is often referred to as an <strong>electrostatic force <\/strong>.\u00a0 An <strong>ionic bond <\/strong>is the electrostatic force that holds ions together in an <strong>ionic<\/strong><strong>compound <\/strong>. \u00a0The strength of the ionic bond is directly dependent upon the quantity of the charges and inversely dependent on the distance between the charged particles.\u00a0 A cation with a 2+ charge will make a stronger ionic bond than a cation with a 1+ charge.\u00a0 A larger ion makes a weaker ionic bond because of the greater distance between its electrons and the nucleus of the oppositely charged ion.<\/p>\r\n\r\n<h4>Electron Dot Diagrams<\/h4>\r\n<p id=\"x-ck12-OGU4MjhkNGFhZWNmYmJjNjg1ZDc0ODk2NThiZjk2NWQ.-6jn\">We will use sodium chloride as an example to demonstrate the nature of the ionic bond and how it forms.\u00a0 As you know, sodium is a metal and loses its one valence electron to become a cation.\u00a0 Chlorine is a nonmetal and gains one electron in becoming an anion.\u00a0 Both achieve a noble-gas electron configuration.\u00a0 However, electrons cannot be simply \u201clost\u201d to nowhere in particular.\u00a0 A more accurate way to describe what is happening is that a single electron is transferred from the sodium atom to the chlorine atom as shown below.<\/p>\r\n<p id=\"x-ck12-MTQ2NmIzNTQ2MWJlZmRhNTEzNTE1NzNiYTQ1NjIyYjY.-2ku\"><span class=\"x-ck12-img-inline\"><img src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images-archive-read-only\/wp-content\/uploads\/sites\/53\/2014\/08\/19211356\/20140811155231762418.png\" alt=\"Transfer of an electron from sodium to chlorine to form sodium chloride\" width=\"250\" \/><\/span><\/p>\r\n<p id=\"x-ck12-YjlkOWQzZjM3M2ZiYTk5ZjlkNmUwZjdmYmNkNWJmMGE.-wzn\">The ionic bond is the attraction of the Na <sup>+ <\/sup>ion for the Cl <sup>\u2212 <\/sup>ion.\u00a0 It is conventional to show the cation without dots around the symbol to emphasize that the original energy level that contained the valence electron is now empty.\u00a0 The anion is now shown with a complete octet of electrons.<\/p>\r\n<p id=\"x-ck12-ZmQwMTk5MTU4NGU2OTY2ZjhmODBhNmExYWUzMDcwOGU.-wb8\">For a compound such as magnesium chloride, it is not quite as simple.\u00a0 Because magnesium has two valence electrons, it needs to lose both to achieve the noble-gas configuration.\u00a0 Therefore, two chlorine atoms will be needed.<\/p>\r\n<p id=\"x-ck12-NTU5Y2MxNWQzZTUxZWM5ZTM0MjgzOWIyMjhjM2YxYWE.-fnt\"><span class=\"x-ck12-img-inline\"><img src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images-archive-read-only\/wp-content\/uploads\/sites\/53\/2014\/08\/19211358\/20140811155231903185.png\" alt=\"Transfer of electrons from magnesium to chlorines to form magnesium chloride\" width=\"250\" \/><\/span><\/p>\r\n<p id=\"x-ck12-NTU5Y2MxNWQzZTUxZWM5ZTM0MjgzOWIyMjhjM2YxYWE.-qol\">The final formula for magnesium chloride is MgCl <sub>2 <\/sub>.<\/p>\r\n\r\n<h4>Summary<\/h4>\r\n<ul id=\"x-ck12-OTlhYjU3NDQ1OThjY2RiNzBiYThjZTczZjE1N2Q1MGU.-lcg\">\r\n \t<li>An ionic compound contains positive and negative ions.<\/li>\r\n \t<li>An ionic bond is electrostatic in nature.<\/li>\r\n \t<li>Electron dot diagrams can be used to illustrate electron movements and ion formation.<\/li>\r\n<\/ul>\r\n<h4>Practice<\/h4>\r\n<p id=\"x-ck12-NmNlM2JkYzM5ZTU0NDcyNTAzOGUwZTg3Yjc3MWRiMWU.-x3b\"><em>Questions<\/em><\/p>\r\n<p id=\"x-ck12-Y2JlMjQ5M2YzMTNmNmRjMzNmZTI0MTMzYzcwM2IzZmY.-kcr\">Look at this <a href=\"https:\/\/web.archive.org\/web\/20100614023230\/http:\/\/chemed.chem.wisc.edu\/chempaths\/GenChem-Textbook\/Ionic-Bonding-565.html\" target=\"_blank\" rel=\"noopener\">page on Ionic Bonding<\/a> to answer the following questions:<\/p>\r\n\r\n<ol id=\"x-ck12-YWViZThmNjBmNDM3M2ZiZTcwNmI4YTJlMjk2ZTAyNDA.-krt\">\r\n \t<li>What do cations and anions form?<\/li>\r\n \t<li>What influences attraction for electrons?<\/li>\r\n \t<li>What metals generally form ionic bonds?<\/li>\r\n<\/ol>\r\n<h4>Review<\/h4>\r\n<p id=\"x-ck12-NmNlM2JkYzM5ZTU0NDcyNTAzOGUwZTg3Yjc3MWRiMWU.-avc\"><em>Questions<\/em><\/p>\r\n\r\n<ol id=\"x-ck12-ZTE2NDJmNzg2MzllYTE1MjMxMzU3MTdlOGQ0ZWJkYjc.-1r2\">\r\n \t<li>What is an ionic compound?<\/li>\r\n \t<li>What is an ionic bond?<\/li>\r\n \t<li>Which cation (Na <sup>+ <\/sup>or Ca <sup>2+ <\/sup>) would form a stronger ionic bond with Cl <sup>-<\/sup><\/li>\r\n<\/ol>\r\n<div class=\"x-ck12-data-problem-set\"><\/div>\r\n<div class=\"x-ck12-data-vocabulary\">\r\n<ul id=\"x-ck12-YWMxZWYzMTA5MzA2YzE4NWJjY2RiZTM3MDc5NWY5YzI.-r9e\">\r\n \t<li><strong>electrostatic force: <\/strong>Attraction of oppositely charged particles toward one another.<\/li>\r\n \t<li><strong>ionic bond: <\/strong>The electrostatic force that holds ions together in an ionic compound.<\/li>\r\n \t<li><strong>ionic compound: <\/strong>An electrically neutral compound consisting of positive and negative ions.<\/li>\r\n<\/ul>\r\n<\/div>\r\n<h1><\/h1>\r\n[reveal-answer q=\"836080\"]Show References[\/reveal-answer]\r\n[hidden-answer a=\"836080\"]\r\n<h2>References<\/h2>\r\n<ul>\r\n \t<li>Leon Brooks. <a href=\"http:\/\/commons.wikimedia.org\/wiki\/File:Wanneroo_Beach-dsc20050514_155534_24.jpg\"> http:\/\/commons.wikimedia.org\/wiki\/File:Wanneroo_Beach-dsc20050514_155534_24.jpg <\/a> .<\/li>\r\n \t<li>CK-12 Foundation - Joy Sheng.<\/li>\r\n \t<li>CK-12 Foundation - Joy Sheng.<\/li>\r\n<\/ul>\r\n[\/hidden-answer]","rendered":"<h1 id=\"x-ck12-SW9uaWMgYW5kIE1ldGFsbGljIEJvbmRpbmc.-chapter\">Ionic and Metallic Bonding<\/h1>\n<div class=\"x-ck12-data\"><\/div>\n<h1 id=\"x-ck12-RWxlY3Ryb24gRG90IERpYWdyYW1z\">Ionic Bonding<\/h1>\n<div class=\"x-ck12-data-objectives\">\n<ul id=\"x-ck12-Y2Q1MjBiMGQ3YjQxMjUxNWNmODU0N2IxZjliZGU3N2U.-il7\">\n<li>Define ionic compound.<\/li>\n<li>Define ionic bond.<\/li>\n<li>Use electron dot diagrams to illustrate electron transfer and ionic bond formation.<\/li>\n<\/ul>\n<\/div>\n<p id=\"x-ck12-ZmQ0Y2JmYmY3YzI2ODA0ODhhYTFlYTdjMTI0ZGIzZTk.-vbk\"><span class=\"x-ck12-img-inline\"><img decoding=\"async\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images-archive-read-only\/wp-content\/uploads\/sites\/53\/2014\/08\/19211355\/20140811155231639993.jpeg\" alt=\"The sea contains a lot of salt, an ionic compound\" width=\"400\" \/><\/span><\/p>\n<p id=\"x-ck12-YTc2OWI2OTFjNmIwMWFlOTM5MTZhYWJkNTRjYzMzMDc.-rsp\"><strong>Does the sea really have salt in it?<\/strong><\/p>\n<p id=\"x-ck12-MDRhZDIxNWFjMTRjOGQ2YjBmYjMzOGExNmUzZTQ0NTE.-c1w\">We can get common table salt from several sources.\u00a0 It can be mined in the solid form in salt mines or found as a solid in deposits.\u00a0 We can also get salt from the ocean, but it really does not exist as salt when in solution.\u00a0 The sodium ions and chloride ions are dissolved, but not combined into a structure until all the water is removed.<\/p>\n<p id=\"x-ck12-OGExYWVjNDUzMTk5ODEyZTdkMzBlYzJmMDkzYmNjYmU.-icq\">Most of the rocks and minerals that make up the Earth\u2019s crust are composed of positive and negative ions held together by ionic bonding.\u00a0 An ionic compound is an electrically neutral compound consisting of positive and negative ions.\u00a0 You are very familiar with some ionic compounds such as sodium chloride (NaCl).\u00a0 A sodium chloride crystal consists of equal numbers of positive sodium ions (Na <sup>+ <\/sup>) and negative chloride ions (Cl <sup>\u2212 <\/sup>).\u00a0 <em>\u00a0<\/em><\/p>\n<h3>Ionic Bonds<\/h3>\n<p id=\"x-ck12-MWMxM2E0NmY3MmZkNzQ1YjdmY2Y0Y2IyODU5OTBkNmI.-ez1\">Oppositely charged particles attract each other.\u00a0 This attractive force is often referred to as an <strong>electrostatic force <\/strong>.\u00a0 An <strong>ionic bond <\/strong>is the electrostatic force that holds ions together in an <strong>ionic<\/strong><strong>compound <\/strong>. \u00a0The strength of the ionic bond is directly dependent upon the quantity of the charges and inversely dependent on the distance between the charged particles.\u00a0 A cation with a 2+ charge will make a stronger ionic bond than a cation with a 1+ charge.\u00a0 A larger ion makes a weaker ionic bond because of the greater distance between its electrons and the nucleus of the oppositely charged ion.<\/p>\n<h4>Electron Dot Diagrams<\/h4>\n<p id=\"x-ck12-OGU4MjhkNGFhZWNmYmJjNjg1ZDc0ODk2NThiZjk2NWQ.-6jn\">We will use sodium chloride as an example to demonstrate the nature of the ionic bond and how it forms.\u00a0 As you know, sodium is a metal and loses its one valence electron to become a cation.\u00a0 Chlorine is a nonmetal and gains one electron in becoming an anion.\u00a0 Both achieve a noble-gas electron configuration.\u00a0 However, electrons cannot be simply \u201clost\u201d to nowhere in particular.\u00a0 A more accurate way to describe what is happening is that a single electron is transferred from the sodium atom to the chlorine atom as shown below.<\/p>\n<p id=\"x-ck12-MTQ2NmIzNTQ2MWJlZmRhNTEzNTE1NzNiYTQ1NjIyYjY.-2ku\"><span class=\"x-ck12-img-inline\"><img decoding=\"async\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images-archive-read-only\/wp-content\/uploads\/sites\/53\/2014\/08\/19211356\/20140811155231762418.png\" alt=\"Transfer of an electron from sodium to chlorine to form sodium chloride\" width=\"250\" \/><\/span><\/p>\n<p id=\"x-ck12-YjlkOWQzZjM3M2ZiYTk5ZjlkNmUwZjdmYmNkNWJmMGE.-wzn\">The ionic bond is the attraction of the Na <sup>+ <\/sup>ion for the Cl <sup>\u2212 <\/sup>ion.\u00a0 It is conventional to show the cation without dots around the symbol to emphasize that the original energy level that contained the valence electron is now empty.\u00a0 The anion is now shown with a complete octet of electrons.<\/p>\n<p id=\"x-ck12-ZmQwMTk5MTU4NGU2OTY2ZjhmODBhNmExYWUzMDcwOGU.-wb8\">For a compound such as magnesium chloride, it is not quite as simple.\u00a0 Because magnesium has two valence electrons, it needs to lose both to achieve the noble-gas configuration.\u00a0 Therefore, two chlorine atoms will be needed.<\/p>\n<p id=\"x-ck12-NTU5Y2MxNWQzZTUxZWM5ZTM0MjgzOWIyMjhjM2YxYWE.-fnt\"><span class=\"x-ck12-img-inline\"><img decoding=\"async\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images-archive-read-only\/wp-content\/uploads\/sites\/53\/2014\/08\/19211358\/20140811155231903185.png\" alt=\"Transfer of electrons from magnesium to chlorines to form magnesium chloride\" width=\"250\" \/><\/span><\/p>\n<p id=\"x-ck12-NTU5Y2MxNWQzZTUxZWM5ZTM0MjgzOWIyMjhjM2YxYWE.-qol\">The final formula for magnesium chloride is MgCl <sub>2 <\/sub>.<\/p>\n<h4>Summary<\/h4>\n<ul id=\"x-ck12-OTlhYjU3NDQ1OThjY2RiNzBiYThjZTczZjE1N2Q1MGU.-lcg\">\n<li>An ionic compound contains positive and negative ions.<\/li>\n<li>An ionic bond is electrostatic in nature.<\/li>\n<li>Electron dot diagrams can be used to illustrate electron movements and ion formation.<\/li>\n<\/ul>\n<h4>Practice<\/h4>\n<p id=\"x-ck12-NmNlM2JkYzM5ZTU0NDcyNTAzOGUwZTg3Yjc3MWRiMWU.-x3b\"><em>Questions<\/em><\/p>\n<p id=\"x-ck12-Y2JlMjQ5M2YzMTNmNmRjMzNmZTI0MTMzYzcwM2IzZmY.-kcr\">Look at this <a href=\"https:\/\/web.archive.org\/web\/20100614023230\/http:\/\/chemed.chem.wisc.edu\/chempaths\/GenChem-Textbook\/Ionic-Bonding-565.html\" target=\"_blank\" rel=\"noopener\">page on Ionic Bonding<\/a> to answer the following questions:<\/p>\n<ol id=\"x-ck12-YWViZThmNjBmNDM3M2ZiZTcwNmI4YTJlMjk2ZTAyNDA.-krt\">\n<li>What do cations and anions form?<\/li>\n<li>What influences attraction for electrons?<\/li>\n<li>What metals generally form ionic bonds?<\/li>\n<\/ol>\n<h4>Review<\/h4>\n<p id=\"x-ck12-NmNlM2JkYzM5ZTU0NDcyNTAzOGUwZTg3Yjc3MWRiMWU.-avc\"><em>Questions<\/em><\/p>\n<ol id=\"x-ck12-ZTE2NDJmNzg2MzllYTE1MjMxMzU3MTdlOGQ0ZWJkYjc.-1r2\">\n<li>What is an ionic compound?<\/li>\n<li>What is an ionic bond?<\/li>\n<li>Which cation (Na <sup>+ <\/sup>or Ca <sup>2+ <\/sup>) would form a stronger ionic bond with Cl <sup>&#8211;<\/sup><\/li>\n<\/ol>\n<div class=\"x-ck12-data-problem-set\"><\/div>\n<div class=\"x-ck12-data-vocabulary\">\n<ul id=\"x-ck12-YWMxZWYzMTA5MzA2YzE4NWJjY2RiZTM3MDc5NWY5YzI.-r9e\">\n<li><strong>electrostatic force: <\/strong>Attraction of oppositely charged particles toward one another.<\/li>\n<li><strong>ionic bond: <\/strong>The electrostatic force that holds ions together in an ionic compound.<\/li>\n<li><strong>ionic compound: <\/strong>An electrically neutral compound consisting of positive and negative ions.<\/li>\n<\/ul>\n<\/div>\n<h1><\/h1>\n<div class=\"qa-wrapper\" style=\"display: block\"><span class=\"show-answer collapsed\" style=\"cursor: pointer\" data-target=\"q836080\">Show References<\/span><\/p>\n<div id=\"q836080\" class=\"hidden-answer\" style=\"display: none\">\n<h2>References<\/h2>\n<ul>\n<li>Leon Brooks. <a href=\"http:\/\/commons.wikimedia.org\/wiki\/File:Wanneroo_Beach-dsc20050514_155534_24.jpg\"> http:\/\/commons.wikimedia.org\/wiki\/File:Wanneroo_Beach-dsc20050514_155534_24.jpg <\/a> .<\/li>\n<li>CK-12 Foundation &#8211; Joy Sheng.<\/li>\n<li>CK-12 Foundation &#8211; Joy Sheng.<\/li>\n<\/ul>\n<\/div>\n<\/div>\n","protected":false},"author":1507,"menu_order":7,"template":"","meta":{"_candela_citation":"[]","CANDELA_OUTCOMES_GUID":"","pb_show_title":"on","pb_short_title":"","pb_subtitle":"","pb_authors":[],"pb_section_license":""},"chapter-type":[],"contributor":[],"license":[],"class_list":["post-2794","chapter","type-chapter","status-publish","hentry"],"part":2329,"_links":{"self":[{"href":"https:\/\/courses.lumenlearning.com\/umes-cheminter\/wp-json\/pressbooks\/v2\/chapters\/2794","targetHints":{"allow":["GET"]}}],"collection":[{"href":"https:\/\/courses.lumenlearning.com\/umes-cheminter\/wp-json\/pressbooks\/v2\/chapters"}],"about":[{"href":"https:\/\/courses.lumenlearning.com\/umes-cheminter\/wp-json\/wp\/v2\/types\/chapter"}],"author":[{"embeddable":true,"href":"https:\/\/courses.lumenlearning.com\/umes-cheminter\/wp-json\/wp\/v2\/users\/1507"}],"version-history":[{"count":6,"href":"https:\/\/courses.lumenlearning.com\/umes-cheminter\/wp-json\/pressbooks\/v2\/chapters\/2794\/revisions"}],"predecessor-version":[{"id":3642,"href":"https:\/\/courses.lumenlearning.com\/umes-cheminter\/wp-json\/pressbooks\/v2\/chapters\/2794\/revisions\/3642"}],"part":[{"href":"https:\/\/courses.lumenlearning.com\/umes-cheminter\/wp-json\/pressbooks\/v2\/parts\/2329"}],"metadata":[{"href":"https:\/\/courses.lumenlearning.com\/umes-cheminter\/wp-json\/pressbooks\/v2\/chapters\/2794\/metadata\/"}],"wp:attachment":[{"href":"https:\/\/courses.lumenlearning.com\/umes-cheminter\/wp-json\/wp\/v2\/media?parent=2794"}],"wp:term":[{"taxonomy":"chapter-type","embeddable":true,"href":"https:\/\/courses.lumenlearning.com\/umes-cheminter\/wp-json\/pressbooks\/v2\/chapter-type?post=2794"},{"taxonomy":"contributor","embeddable":true,"href":"https:\/\/courses.lumenlearning.com\/umes-cheminter\/wp-json\/wp\/v2\/contributor?post=2794"},{"taxonomy":"license","embeddable":true,"href":"https:\/\/courses.lumenlearning.com\/umes-cheminter\/wp-json\/wp\/v2\/license?post=2794"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}